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The pressure exerted by 1 mol of CO(2) a...

The pressure exerted by 1 mol of `CO_(2)` at `273 K` is `34.98 atm`. Assuming that volume occupied by `CO_(2)` molecules is negligible, the value of van der Waal's constant for attraction of `CO_2` gas is

A

`3.59 dm^(6)atm mol^(-2)`

B

`2.59 dm^(6)atm mol^(-2)`

C

`1.25 dm^(6)atm mol^(-2)`

D

`1.59 dm^(6)atm mol^(-2)`

Text Solution

Verified by Experts

The correct Answer is:
A
`[P+(a)/(V^2)][V-a]= RT`. When volume of `CO_(2)` molecules is negligible, `[P+(a)/(V^2)]V= RT" or "V^(2)P-RTV+a= 0`
`V= (+RT pm sqrt(R^(2)T^(2)-4Pa))/(2P)`
Since, V is constant at given P and T, V can have only one value or discriminant = 0
`therefore R^(2)T^(2)= 4Pa" or "a= (R^(2)T^(2))/(4P)= ((0.0821)^(2)xx(273)^(2))/(4xx 34.98)= 3.59 dm^(6) atm mol^(-2)`.
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